Equilibrium Constants and Water Activity RevisitedDavid KeeportsSubtle arguments based upon the use of chemical potentials show that numerical values of solute molar concentrations can be used as good approximate activities in equilibrium calculations for reactions involving dilute solutions.Keeports, David. J. Chem. Educ.2006, 83, 1290.

pH Paradoxes: Demonstrating That It Is Not True That pH ≡ -log[H+]Christopher G. McCarty and Ed VitzSix demonstrations highlighting paradoxes that arise if pH is incorrectly defined as -log[H+] are presented as justification for the recommendation that pH should be correctly defined as pH = -log aH+ in textbooks.McCarty, Christopher G.; Vitz, Ed. J. Chem. Educ.2006, 83, 752.

Acids / Bases |

Aqueous Solution Chemistry |

Ion Selective Electrodes |

pH |

Quantitative Analysis

Teaching pH Measurements with a Student-Assembled Combination Quinhydrone ElectrodeFritz Scholz, Tim Steinhardt, Heike Kahlert, Jens R. Pörksen, and Jürgen BehnertA combination pH electrode that can be assembled by the student is described. It consists of a glass holder and two sensors in the form of rubber stoppers that contain quinhydrone and graphite. The combination electrode is suitable to teach potentiometric measurements, pH measurements, and the interplay of acidbase and redox equilibria. The electrode meets highest safety standards and overcomes the troubles associated with the use of the conventional quinhydrone electrode.Scholz, Fritz; Steinhardt, Tim; Kahlert, Heike; Pörksen, Jens R.; Behnert, Jürgen. J. Chem. Educ.2005, 82, 782.

Acids / Bases |

pH |

Laboratory Equipment / Apparatus |

Electrochemistry

The Relative Acidities of Water and MethanolHenry I. AbrashAnalysis of the disparity between the way the acidity constant of water is presented in general chemistry and organic chemistry textbooks.Abrash, Henry I. J. Chem. Educ.2001, 78, 1496.

Acids / Bases |

Equilibrium

Acids and Bases in Layers: The Stratal Structure of an Ancient TopicWobbe de Vos and Albert PilotThis article identifies and discusses six successive "layers" that can be recognized in chapters on acids and bases in general chemistry textbooks, each the result of what once was a modernization; the cumulative result of these layers has become problematic, and some learning problems that students have when studying acids and bases become comprehensible when viewed from this perspective. de Vos, Wobbe; Pilot, Albert. J. Chem. Educ.2001, 78, 494.

Acids / Bases |

Learning Theories |

Lewis Acids / Bases |

Brønsted-Lowry Acids / Bases

Do pH in Your HeadAddison AultEvery aqueous solution has a pH. Two factors determine this pH: the acidic or basic strength of the solute, and its concentration. When you use pKa values to express acidic and basic strength you can easily estimate the approximate pH of many aqueous solutions of acids, bases, and their salts and their buffers.Ault, Addison. J. Chem. Educ.1999, 76, 936.

Quality levels and the Brønsted theoryBank, EvelynMaintaining standards for a diversity of students and teaching hydrolysis with the Bronsted-Lowry theory. [Debut]Bank, Evelyn J. Chem. Educ.1977, 54, 548.

Acids / Bases |

Aqueous Solution Chemistry |

Brønsted-Lowry Acids / Bases

Beginning chemistry can be relevantCorwin, James F.The continuing criticism offered by students of the science that the present day courses are not relevant to contemporary problems. This can be answered in part by a laboratory program based on environmental problems.Corwin, James F. J. Chem. Educ.1971, 48, 522.

Computer programs for calculating pHSchlessinger, Gert G.A brief note on the availability of a Fortran II program for calculating the pH of weak acids and bases and salts of these species in aqueous solution.Schlessinger, Gert G. J. Chem. Educ.1969, 46, 680.

Acids / Bases |

pH |

Aqueous Solution Chemistry

Chemical queries. Especially for introductory chemistry teachersYoung, J. A.; Malik, J. G.(1) Is there such a thing as a negative pH value? Or one above 14? (2) What is entropy, in terms a beginner may understand? (3) On calculating the molecular weight of a solute from concentration and freezing point depression.Young, J. A.; Malik, J. G. J. Chem. Educ.1969, 46, 36.

Acids / Bases |

Aqueous Solution Chemistry |

pH |

Thermodynamics |

Molecular Properties / Structure

Teaching ionic equilibrium: Use of log chart transparenciesFreiser, Henry; Fernando, QuintusThe use of graphical methods brings the problem of significance of various terms in complicated expressions into proper focus. Furthermore, a pictorial representation permits the student to see at a glance how the concentrations of various species in a system at equilibrium change with conditions.Freiser, Henry; Fernando, Quintus J. Chem. Educ.1965, 42, 35.

Aqueous Solution Chemistry |

Equilibrium |

Acids / Bases |

pH |

Chemometrics |

Brønsted-Lowry Acids / Bases

Sulfuric acid and the hydrated hydronium ionJurale, BernardDescribes how the sulfuric acid-water system can be used to establish the identity of the hydronium and hydrated hydronium ions.Jurale, Bernard J. Chem. Educ.1964, 41, 573.

Acids / Bases |

Aqueous Solution Chemistry |

Phases / Phase Transitions / Diagrams

The hydrated hydronium ionClever, H. LawrenceIt is the purpose of this brief review to cite and discuss some of the evidence for the existence of the trihydrated hydronium ion.Clever, H. Lawrence J. Chem. Educ.1963, 40, 637.

Potentiometric measurements of equilibria: In general chemistry laboratoryChesick, J. P.; Patterson, Andrew, Jr.The authors describe an experiment in which the solubility product of silver chloride, the ionization constant of the silver-ammonia complex, and the ionization constant of acetic acid can be determined with one afternoon of work.Chesick, J. P.; Patterson, Andrew, Jr. J. Chem. Educ.1959, 36, 496.

Electrochemistry |

Equilibrium |

Precipitation / Solubility |

Aqueous Solution Chemistry |

Acids / Bases

Amphoteric molecules, ions and saltsDavidson, DavidIt is the aim of this paper to call attention to the splendid opportunity amphoteric substances afford for the teaching of acid-base principles.Davidson, David J. Chem. Educ.1955, 32, 550.